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CHAPTER+5_Drill

# CHAPTER+5_Drill - CHAPTER 5_Drills Gas 1(a List the four...

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CHAPTER 5_Drills/ Gas 1. (a) List the four parameters used to describe the behavior of a gas: (b) What are the principal assumptions of the Kinetic-Molecular Theory? (c) How is Boyle’s law related to the ideal gas law? (d) How is Charles’ law related to the ideal gas law? (e) How is the combined gas law related to the ideal gas law? (b) Under what condition of temperature and pressure, is a gas least likely to exhibit ideal behavior? Explain. 2. Fill in the blank. True (T) or False (F). Compare at the same T and P, equal volume of H 2 and O 2 has When constant volume is maintained, what effect does heating 1 mole of O 2 gas have on (I: increase; D: decrease; NE: effect) The same number of molecules Its density The same mass Its mass The same density Its pressure the same average velocity The average kinetic energy of its molecules The same average kinetic energy of its molecules The average rms speed of its molecules The same average rms speed The rate of effusion of its molecules The same rate of effusion The number of O 2 in the sample 3. Sketch. P V T V P T V n (a) Constant T and n (b) Constant P and n (c) Constant V and n (d) Constant T and P

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4. A sample of a gas occupies a volume of 635 mL at 722 torr. At constant temperature, what will be the new volume when the pressure changes to the following: a) 2.5 atm ( Ans. 241 mL ) b) 795 mmHg ( Ans. 577 mL ) 5. Given 6.00 L of N 2 gas at 25°C, what volume will the nitrogen occupy at (a) 0.0°F? (b) 345. K? (Assume constant pressure.) ( Ans. 6.17 L; 8.35 L ) 6. A bicycle tire is filled with air to a pressure of 610 kPa, at a temperature of 19 °C. Riding the bike on asphalt on a hot day increases the temperature to 58 °C. The volume of the tire increases by 4.0%. What is the new pressure in the tire? ( Ans. 665 kPa ) 7. A high vacuum pump can produce a pressure of 1.0 × 10 -6 Torr. How many molecules are in each mL of gas at 25 °C at this low
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CHAPTER+5_Drill - CHAPTER 5_Drills Gas 1(a List the four...

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